31. Predict which substance in each of the following pairs would have the greater intermolecular forces. a. CO_(2) or OCS b. SeO_(2) or SO_(2) C. CH_(3)CH_(2)CH_(2)NH_(2) or H_(2)NCH_(2)CH_(2)NH_(2) d. CH_(3)CH_(3) or H_(2)CO e. CH_(3)OH or H_(2)CO 32. Consider the compounds Cl_(2),HCl,F_(2) , NaF, and HF . Which com- pound has a boiling point closest to that of argon?Explain.

31. a. would have greater intermolecular forces than because it has a polar covalent bond due to the difference in electronegativity between oxygen and carbon, leading to dipole-dipole interactions.b. would have greater intermolecular forces than because sulfur is smaller than selenium, resulting in stronger dipole-dipole interactions.c. would have greater intermolecular forces than because the presence of the additional methyl group ( ) increases the surface area and the number of electrons available for van der Waals forces.d. would have greater intermolecular forces than because it has a polar covalent bond due to the difference in electronegativity between carbon and oxygen, leading to dipole-dipole interactions.e. would have greater intermolecular forces than because it has a polar covalent bond due to the difference in electronegativity between carbon and oxygen, and it also has hydrogen bonding between the hydrogen atom of the hydroxyl group and the oxygen atom.32. Among the given compounds, has a boiling point closest to that of argon. This is because argon is a noble gas with a very low boiling point, and , being a diatomic molecule with nonpolar covalent bonds, also has a low boiling point due to weak van der Waals forces between the molecules.